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Continue Acetic redirects here. This should not be confused with Ascetic. colorless and weak liquid organic compounds found in vinegar acetic acid vinegar Names Preferred IUPAC name vinegar named vinegar vinegar (when diluted); Hydrogen acetate; Метанкарбоксиловая кислота (JSmol) Идентификаторы CAS Номер 64-19-7 Y 3D модель (JSmol) Интерактивное изображение 3DMet B00009 Аббревиатуры AcOH Beilstein Справка 506007 ChEBI CHEBI:15366 Y ChEMBL ChEMBL539 Y ChemSpider Y ChemSpider171 Y DrugBank DB03166 Y ECHA InfoCard 100.000.528 EC Номер 200-580-7 E номер E260 (консерванты) Gmelin Справка 1380 IUPHAR/BPS 1058 KEGG D00010 N MeSH Acetic кислота PubChem CID 176 RTECS номер AF1225000 UNII No40-9N063P Y UN номер 2789 CompTox Dashboard (EPA) DTXSID5024394 InChI InChI-1S/C2H4O2/c1-2(3)4/h1H3,((H.3,4) YKey: «ТБСБХВТЕАМЕЗО-УФФФАОЯ-Н Y SMILES CC(O)»O Свойства Химическая формула C2H4O2 Молар масса 60,052 г»mol-1 Внешний вид Бесцветная жидкость Odor Heavily уксус-как Плотность 1.049 г см-3 (жидкость); 1,27 г см3 (твердая) точка плавления от 16 до 17 градусов по Цельсию; от 61 до 62 градусов по Фаренгейту; от 289 до 290 K Точка кипения от 118 до 119 градусов по Цельсию; от 244 до 246 градусов по Фаренгейту; 391 to 392 K Solubility in water Miscible log P - 0.28[4] Acidity (pKa) 4.756 (H2O)[5]12.6 (DMSO)[6] Basicity (pKb) 9.24 (basicity of acetate ion) Conjugate base Acetate Magnetic susceptibility (χ) -31.54·10−6 cm3/mol Refractive index (nD) 1.371 (VD = 18.19) Viscosity 1.22 mPa s Dipole moment 1.74 D Thermochemistry Heat capacity (C) 123.1 J K−1 mol−1 Std molarentropy (So298) 158.0 J K−1 mol−1 Std enthalpy offormation (ΔfH⦵298) -483.88–483.16 kJ mol−1 Std enthalpy ofcombustion (ΔcH⦵298) -875.50– 874.82 kJ mol−1 Pharmacology ATC code G01AD02 (WHO) S02AA10 (WHO) Hazards Safety data sheet See: data page GHS pictograms GHS Signal word Danger GHS hazard statements H226, H314 GHS precautionary statements P280, P305+351+338, P310 NFPA 704 (fire diamond) 2 3 0 Flash point 40 °C (104 °F; 313 K) Autoignitiontemperature 427 °C (801 °F; 700 K) Explosive limits 4–16% Lethal dose or concentration (LD , LC): LD50 (medium dose) 3.31 g kg No.1, oral (rat) LC50 (average concentration) 5620 ppm (mouse, 1 hour)16,000 ppm (rat, 4 hours) NIOSH (U.S. health impact restrictions): PEL (acceptable) TWA 10 ppm (25 mg/m3) REL (Recommended) TWA 10 ppm (25 mg/m3) ST 15 ppm (37 mg/m3) Associated Compounds Associated Carboxyline Acid Formic acidPropionic acid Associated Compounds Acetaldehyde Acetamide Acetatid acetatid A Acetonide acetone atcetonitril Acetylchloride ethanol ethyl potassium acetate acetate acetate tioacetic acid Additional data page Structure and Entrepreneurs Refractive Index (n). Thermodynamic Data Behavior Phase of The Solid-Liquid-Gas Spectral Data OF UV, IR, JMR, MS Except when otherwise noted, data are given materials in their standard state (at 25 degrees Celsius, Celsius, N check (what is YN?) Infobox refers to acetic acid /əˈsiːtɪk/, systematically referred to as ethanol /ˌɛθəˈnoʊɪk/, is a colorless liquid organic compound with the chemical formula CH3COOH (also written as CH3CO2H, C2H4O2, or HC2H3O2). When undiluted, it is sometimes called glacial acetic acid. Vinegar is at least 4% acetic acid by volume, making acetic acid the main component of vinegar other than water. Vinegar acid has a characteristic sour taste and pungent smell. In addition to household vinegar, it is mainly produced as a precursor to polyvinyl acetate and cellulose acetate. It is classified as a weak acid, as it is only partially disassociated in the solution, but concentrated acetic acid is corrosive and can attack the skin. Acetic acid is the second simplest carboxic acid (after cream acid). It consists of a methyl group attached to the carboxil group. It is an important chemical reagent and industrial chemical used mainly in the production of cellulose acetate for film, polyvinyl acetate for wood glue, as well as synthetic fibers and tissues. In households, diluted acetic acid is often used in descaling agents. In the food industry, acetic acid is controlled by the E260 food additive code as a regulator of acidity and as a condiment. In biochemistry, the acetyl group derived from acetic acid is fundamental to all life forms. When tied to Coenzyme A, it is central to the metabolism of carbohydrates and fats. The global demand for acetic acid is about 6.5 million metric tons per year (Mt/a), of which approximately 1.5 Mt/a is processed; the rest is made from methanol. Vinegar mainly dilutes acetic acid, often produced by fermentation and subsequent ethanol oxidation. The trivial name for acetic acid is the most commonly used and preferred name of IUPAC. The systematic name of ethanol, the real name IUPAC, is built in accordance with the replacement nomenclature. The name acetic acid comes from acetum, the Latin word for vinegar, and is associated with the word acid itself. Glacial acetic acid is the name of acetic acid, free of water (anhydrous). Similar to the German name Eisessig (ice vinegar), the name comes from ice crystals that form just below room temperature at 16.6 degrees Celsius (61.9 degrees Fahrenheit) (the presence of 0.1% water reduces the melting point by 0.2 degrees Celsius). A common symbol of acetic acid is AcOH, where Ac is a symbol of pseudo-element, representing the acetyl group CH3-C (ZO); Conjug base, acetate (CH3COO), is thus presented as ACHO. (The Ac is not Confused with the symbol of the element's actification; context prevents confusion among organic chemists). To better reflect its structure, acetic acid is often spelled as CH3-C(O)OH, CH3'C (ZO) OH, CH3COOH, and CH3CO2H. In the context of acid-base reactions, the acronym HAc sometimes sometimes where ac in this case is a symbol of acetate (not acetyla). Acetate ion as a result of the loss of H e from acetic acid. The name acetate may also refer to salt containing this anion, or ester acetic acid. Свойства кристаллов уксусной кислоты Кислотность Водородный центр в карбоксил-группе (COOH) в карбоксилиновых кислотах, таких как уксусная кислота, может отделяться от молекулы ионизацией: CH3COOH ⇌ CH3CO2 Уксусная кислота является слабой монопротической кислотой. In aqueous solution, it has a pKa value of 4.76. Its conjugation base is acetate (CH3COO). Solution 1.0 M (about the concentration of domestic vinegar) has a pH of 2.4, which indicates that only 0.4% of the molecules of acetic acid are separated. However, in a very diluted (10-6 M) acetic acid solution, 90% is dissociated. Cyclical dimer of acetic acid; Dotted green lines represent a hydrogen bond Structure In solid acetic acid, molecules form chains, separate molecules, interconnected hydrogen bonds. Dimers can be found in a pair at 120 degrees Celsius (248 degrees Fahrenheit). Dimers are also found in the liquid phase of diluted solutions in solvents not related to hydrogen, and to some extent in pure acetic acid, but are disturbed by hydrogen solvents. Dissociation of enthalpy dimer is estimated at 65.0-66.0 kJ/mol, and entropy dissociation at 154-157 J mol'1 K'1. Other carboxylic acids are involved in similar intermolecular interactions with hydrogen. Liquid acetic acid solvent properties are hydrophilic (polar) protic solvents similar to ethanol and water. With moderate relative static tolerance (dielectric constant) 6.2, it dissolves not only polar compounds such as inorganic salts and sugars, but also non-polar compounds such as oils as well as polar solutions. It is incorrectly with polar and non-polar solvents such as water, chloroform and hexane. In higher alcans (starting with octane number) acetic acid is not faulty in all compositions, and the salt of acetic acid in alcans is reduced with longer n-alkanes. The properties of solvent and the error of acetic acid make it a useful industrial chemical, for example, as a solvent in the production of dimethyltherepthalate. Biochemistry In physiological pH acetic acid is usually completely ionized for acetate. The acetyl group, formally derived from acetic acid, is fundamental to all life forms. When tied to Coenzyme A, it is central to the metabolism of carbohydrates and fats. Unlike long-range carboxicic acids (fatty acids), acetic acid is not found in natural triglycerides. However, artificial triaceridide triacetin (glycerin triacetate) is a common food supplement and occurs in and topical medicines. Acetic acid is produced and excreted by acetic acid bacteria, in particular, genus Acetobacter and Clostridium acetobutylicum. These bacteria are found everywhere in food, water and soil, and acetic acid is produced naturally as fruits and other foods spoil. Vinegar acid is also a component of vaginal lubrication of humans and other primates, where it appears to serve as a mild antibacterial agent. The plant for the purification and concentration of acetic acid in 1884 is made industrially both synthetically and through bacterial fermentation. About 75% of the acetic acid made for use in the chemical industry is done by carbonylating methanol, explained below. The biological route is only about 10% of the world's production, but it remains important for the production of vinegar, because many food purity laws require vinegar used in food to be biologically original. Other processes include isomerization of methyl format, conversion of singase into acetic acid and oxidation of gas phase ethylene and ethanol. Acetic acid is often a by-product of various reactions, i.e. in the heterogeneous synthesis of catalytic acrylic acid. As of 2003-2005, the total world production of virgin acetic acid was estimated at 5 Mt/a (million tons per year), about half of which was produced in the United States. European production was about 1 Mt/a and declined, while Japanese production was 0.7 Mt/a. Since then, global production has increased to 6.5 Mt/a. Since then, global production has increased to 10.7 Mt/a (in 2010) and beyond; however, this growth is projected to slow. The two largest producers of virgin acetic acid are Celanese and BP Chemicals. Other major manufacturers include Millennium Chemicals, Sterling Chemicals, Samsung, Eastman and Svensk Etanolkemi. Methanol carbonylation Most acetic acid is produced by methanol carbonylation. In this process, methanol and carbon monoxide react to the production of acetic acid according to the equation: the process involves idomeni as an intermediate, and occurs in three stages. Catalyst, metallic carbonyl, is necessary for carbonation (step 2). CH3OH - HI → CH3I - H2O CH3I - CO → CH3COI CH3COI - H2O → CH3COOH - HI Two related methanol carbonation processes: Monsanto's rivima-catalise process and Kativa's iridium-catalise process. The latter process is greener and more efficient and has largely supplanted the first process, often in the same plants. Catalytic amounts of water are used in both processes, but the Cativa process requires less, so the reaction of water and gas shear is suppressed, and fewer by-products are formed. By altering the conditions of the process, acetic anhydride can also be produced at the same plant using rhe birth catalysts. Peridence Prior Prior commercializing the Monsanto process, most of the acetic acid was produced by oxidizing acetaldehyde. This remains the second largest production method, although it is generally not competitive with methanol carbonylation. Acetaldehyde can be produced by moisturizing acetylene. It was the dominant technology of the early 1900s. which decompose to produce acetic acid according to the chemical equation illustrated by butane: 2 C4H10 and 5 O2 → 4 CH3CO2H and 2 H2O Such oxidation require a metal catalyst such as manganese moth salt, cobalt and chromium. A typical reaction is at temperatures and pressures designed to be as hot as possible while retaining butane fluid. Typical reaction conditions are 150 degrees Celsius (302 degrees Fahrenheit) and 55 atm. These by-products are also commercially valuable, and reaction conditions can be changed to produce more of them where necessary. However, separating acetic acid from these sedateds increases the cost of the process. Under similar conditions and using similar catalysts that are used to oxidize butane, oxygen in the air to produce acetic acid can oxidize acetaldehyde. 2 CH3CHO and O2 → 2 CH3CO2H Using modern catalysts, this reaction can have a yield of acetic acid over 95%. The main by-products are ethyl acetate, formal acid and formaldehyde, all of which have lower boiling points than acetic acid, and are easily separated by distillation. Ethylene oxidation of acetaldehyde can be prepared from ethylene through the Wacker process and then oxidized as stated above. Recently, the chemical company Showa Denko, which opened a plant for ethylene oxidation in Tsita, Japan, in 1997, commercialized a cheaper single-etadeform conversion of ethylene into acetic acid. This process is catalyzed by a palladium catalyst supported by heteropolis acid such as silicotungic acid. A similar process used the same metal catalyst on silicutungic acid and silica: 41 C2H4 O2 → CH3CO2H is considered to be competitive with methanol carbonylation for small plants (100-250 ht/a), depending on the local price of ethylene. This approach will be based on the use of new selective photocatalytic oxidation technology for selective oxidation of ethylene and ethane acetic acid. Unlike traditional oxidation catalysts, the selective oxidation process will use UV radiation to produce acetic acid at ambient temperature and pressure. Oxidative fermentation For most of human history, the bacteria acetic acid of the genus Acetobacter made acetic acid, in the form of vinegar. Given amount of oxygen, these bacteria can produce vinegar from a variety of alcoholic alcoholic Commonly used feeds include apple cider, wine and fermented grain, malt, rice or mashed potatoes. The overall chemical reaction is facilitated by these bacteria: C2H5OH and O2 → CH3COOH - H2O diluted alcohol solution, grafted with acetobacter and stored in heat, airy place will become vinegar for several months. Industrial methods of production of vinegar accelerate this process by improving the supply of oxygen to bacteria. The first batches of vinegar produced by fermentation probably followed errors in the winemaking process. If it is necessary to ferment at too high a temperature, acetobacter will suppress yeast occurring naturally on grapes. As demand for vinegar increased for culinary, medical and sanitary purposes, winemakers quickly learned to use other organic materials to produce vinegar during the hot summer months before the grapes were ripe and ready to be processed into wine. This method was slow, however, and not always successful, as winemakers did not understand the process. One of the first modern commercial processes was the fast method or German method first practiced in Germany in 1823. In this process, fermentation takes place in a tower filled with wood chips or charcoal. Alcohol-containing feeds seep into the top of the tower, and fresh air is fed from the bottom either by natural or forced convection. Improving air supply in this process reduce the time to cook vinegar from a few months to a few weeks. Most of the vinegar is now made in the underwater tank culture first described in 1949 by Otto Gromaatka and Heinrich Ebner. In this method, alcohol is fermented to vinegar in a continuously stirred tank, and oxygen is supplied by boiling air through the solution. Using modern uses of this method, vinegar 15% acetic acid can only be prepared within 24 hours in a batch process, even 20% in the 60-hour batch feeding process. Anaerobic enzymatics, including clostridium or Acetobacterium, can convert sugar into acetic acid directly without creating ethanol as an intermediate. The overall chemical reaction of these bacteria can be presented as: C6H12O6 → 3 CH3COOH These acetogenic bacteria produce acetic acid from single-carbon compounds, Including methanol, carbon monoxide, or a mixture of carbon dioxide and hydrogen dioxide: 2 CO2 and 4 H2 → CH3COOH No 2 H2O This ability clostridium to absorb sugar directly, or produce acetic acid from less costly inputs, suggests that these bacteria can produce acetic acid more efficiently than an ethanol oxidizer like Acetobacter. However, Clostridium bacteria are less acid-resistant than acetobacter. Even the most acid-resistant strains can produce vinegar in concentrations of only a few percent, compared to strains of Acetobacter, which can produce vinegar in concentrations of up to 20%. In B it remains more cost effective for producing vinegar using Acetobacter rather than using Clostridium and its concentration. As a result, although acetogenic bacteria have been known since 1940, their industrial use is limited to a few niche applications. Uses acetic acid is a chemical reagent for the production of chemical compounds. The greatest use of acetic acid in the production of vinyl acetate monomer, which is closely watched by vinegar anhydride and esther production. The amount of acetic acid used in vinegar is relatively small. The monomer of vinyl acetate The main use of acetic acid is the production of the acetat vinyl monomer (VAM). In 2008, this app is estimated to consume a third of the world's production of acetic acid. The reaction consists of ethylene and acetic acid with oxygen over the palladium catalyst, carried out in the gas phase. 2 H3C-COOH 2 C2H4 and O2 → 2 H3C-CO-CH2 and 2 H2O Vinyl acetate can be polymerized for polyvinyl acetate or other polymers that are components in paints and glues. The production of Esther's main acetic acid esters are commonly used as solvents for ink, paints and coatings. Ethers include ethyl acetate, acetate n-butila, isobutyl acetate and sawe acetate. They are usually produced by a catalytic reaction of acetic acid and related alcohol: H3C-COOH and HO'R → H3C-CO'O'R H2O, (R - common alkyle group) Most acetate esters, however, are produced from acetaldehyde with the help of Tishchenko's reaction. In addition, essential acetates are used as solvents for nitrocellulose, acrylic varnishes, lacquer and wood stains. First, glycola monoesters are made from ethylene oxide or propylene oxide with alcohol, which are then esterified by acetic acid. The three main products are ethylene glycol monoethyl ester acetate (EEA), ethylene glycol monobutt (EBA) and propylene glycol monometal ester acetate (PMA, better known as PGMEA in semiconductor manufacturing processes, where it is used as a resisting solvent). This app consumes 15% to 20% of the world's acetic acid. Essential acetates, such as the EEA, have shown that they are harmful to human reproduction. Acetic anhydride Product condensation of two molecules of acetic acid is a vinegar anhydride. World production of acetic anhydride is a major application, and uses about 25% to 30% of the world's production of acetic acid. The main process involves dehydrating acetic acid to give keten at 700-750 degrees Celsius. The keten then reacts with acetic acid to obtain → →i anhydride: Thus, its main application is cellulose acetate, synthetic textiles are also used for film. Acetic anhydride is a reagent for heroin and other compounds. The use of glacial acetic acid as a solvent is an excellent polar solvent, as noted above. It is often used as a solvent for re-crystallization to clean organic compounds. Acetic acid is used as a solvent in the production of terephthalic acid (TPA), a raw material for polyethylene terephthalate (PET). In 2006, about 20% of acetic acid was used to produce TPA. Acetic acid is often used as a solvent for reactions associated with carbocracy, such as Friedel-Craft alkyleation. For example, one phase of commercial production of synthetic camphor involves regrouping Kamfen Wagnerian mervein into isobornyl acetate; here the acetic acid acts as a solvent and as a nucleophil to catch the rebuilt carboc. Glacial acetic acid is used in analytical chemistry to assess weakly alkaline substances such as organic amidu. Glacial acetic acid is a much weaker base than water, so amine behaves like a strong base in this environment. It can then be tited with a solution in glacial acetic acid of a very strong acid, such as perchloric acid. Medical article: Injection of acetic acid (medical application) of acetic acid into the tumor has been used to treat cancer since the 1800s. Acid is applied to the cervix, and if the white area appears after about a minute, the test is positive. Acetic acid is an effective antiseptic when used as a 1% solution, with a wide range of activity against streptococcus, staphylococcus, pseudomon, enterococcal and others. It can be used to treat skin infections caused by strains of pseudomonas resistant to typical antibiotics. While diluted acetic acid is used in iontophoresis, no high-quality evidence supports this treatment of rotator cuff disease. As a treatment for otitis externa, it is on the World Health Organization's list of essential medicines, the safest and most effective medicines needed in the health system. Main article Foods: Vinegar acetic acid has 349 kcal per 100 g. Vinegar is usually at least 4% acetic acid by mass. Legal restrictions on acetic acid vary depending on jurisdiction. Vinegar is used directly as a condiment, as well as in the picker of vegetables and other products. Table vinegar tends to be more diluted (4% to 8% acetic acid), while commercial food taking away uses solutions that are more concentrated. The proportion of acetic acid used worldwide as vinegar is not as high as use, but today is the oldest and most known application. Reactions Organic Chemistry acetylchloride SOCl2 acetic acid (i) LiAlH4, ether (ii) H3O ethanol Two typical organic reactions of acetic acid acetic acid undergoing typical chemical reactions of carboxic acid. After treatment base, it is converted into metal acetate and water. With strong bases (such as organolite reagents), it can be doubly deprotoned to give LiCH2CO2Li. Reducing acetic acid gives ethanol. The OH group is the main place of reaction, as evidenced by the conversion of acetic acid into acetylchlorid. Other derivative replacements include acetic anhydride; this anhydride is produced by the loss of water from two molecules of acetic acid. Esters of acetic acid can also be formed through fisher etherization, and amide can be formed. When heated above 440 degrees Celsius (824 degrees Fahrenheit), acetic acid decomposes to → → the production of carbon dioxide and methane, or for the production of keten and water: magnesium and zinc, forming a hydrogen gas and salt called acetate: Mg No. 2 CH3COOH → (CH3COO)2Mg and H2 Because aluminum forms a passive acid-resistant film of aluminum oxide, aluminum tanks are used to transport acetic acid. Metallic acetates can also be prepared from acetic acid and the appropriate base, as in the popular reaction food soda and vinegar: NaHCO3 and CH3COOH → CH3COONa and CO2 H2O Color reaction to salt acetic acid is a solution of iron chloride (III), which leads to a deep red color that disappears after acidification. A more sensitive test uses lantan nitrate with iodine and ammonia to give a blue solution. When hydroced, trioxide forms a kakodyl oxide, which can be detected in its low-odorous vapors. Other derivative organic or inorganic salts are made from acetic acid. Some commercially significant derivatives are sodium acetate, used in the textile industry and as a food preservative (E262). Copper (II) acetate, used as pigment and fungicide. Aluminium acetate and iron (II) acetate, used as muzzles for dyes. Acetate palladium (II), used as a catalyst for organic compound reactions such as Heck reaction. Halogenated acetic acids are made from acetic acid. Some commercially significant derivatives are: (monochloroacetic acid, MCA), dichloroacetic acid (considered a pero- energy product) and trichloroacetic acid. MCA is used in the production of indigo dye. Bromoacetic acid, which is esterified for the production of reagent. Triftoroaceptic acid, which is a common reagent in organic synthesis. The amount of acetic acid used in these other applications together account for another 5-10% of the use of acetic acid worldwide. The history of Vinegar was known in the early civilization as a natural result of the effects of beer and wine in the air, because the bacteria producing vinegar are present all over the world. The use of acetic acid in alchemy extends to the 3rd century BC, when the Greek philosopher Theophrasth described how vinegar acted on metals to produce pigments useful in the including white lead (lead carbonate) and verdigri, a green blend of copper salts including copper acetate (II). The ancient Romans brewed sour wine to produce a very sweet syrup called sapa. The sapa, which was produced in lead pots, was rich in lead acetate, a sweet substance also called lead sugar or Saturn's sugar, which contributed to lead poisoning by the Roman aristocracy. In the 16th century, the German alchemist Andreas Libavis described the production of acetone from the dry distillation of lead acetate, ketonic decarboxylation. The presence of water in vinegar has such a profound effect on the properties of acetic acid that for centuries chemists believed that glacial acetic acid and acid found in vinegar were two different substances. French chemist Pierre Ade proved them identical. Crystallized acetic acid. In 1845, German chemist Hermann Kolbe synthesized acetic acid from inorganic compounds for the first time. This sequence of reactions consisted of chlorination of carbon disulfide to carbon tetrachloride, followed by pyrolysis to tetrachloroethylene and aqueroid chloride trichroacy acid, and culminated in an electrolytic reduction to acetic acid. By 1910, most of the glacial acetic acid was derived from pyrolelic liqueur, a wood distillation product. The acetic acid was secreted by treating lime milk, and as a result calcium acetate was then acidified with sulphuric acid to restore acetic acid. At that time, Germany produced 10,000 tons of glacial acetic acid, about 30% of which was used to produce indigo dye. Since methanol and carbon monoxide are raw materials, methanol-carbonylation has long seemed an attractive precursor to acetic acid. Henri Dreyfus at British Celanese developed a methanol carbonylation plant back in 1925. However, the lack of practical materials that could contain a corrosive reaction mixture at high pressure (200,300 m or more) prevented the commercialization of these routes. The first commercial methanol carbonylation process, which used a cobalt catalyst, was developed by the German chemical company BASF in 1963. In 1968, a rhodic catalyst (cis-Rh(CO)2I2) was discovered that could work effectively at lower pressure with little or no hunting. The American chemical company Monsanto Company built the first plant using this catalyst in 1970, and carbonylation of methanol with the help of rhinous has become the dominant method of production of acetic acid (see Monsanto process). In the late 1990s, the chemical company BP Chemicals commercialized the Cativa catalyst (Ir(CO)2I2), which is promoted by iridium to improve efficiency. This process of catalysis catalysis catalysis greener and more efficient and has largely supplanted the Monsanto process, often at the same manufacturing plants. Interstellar Environment Wednesday The acetic acid was discovered in 1996 by a team led by David Mehringer, using the former Berkeley-Illinois-Maryland Association array at the Hat Creek Radio Observatory and the former Millimeter Massif, located at the Owens Valley Radio Observatory. It was first discovered in the northern molecular cloud sagittarius B2 (also known as the source of the large molecule Sgr B2). Acetic acid is honored to be the first molecule found in interstellar environments using only radio interferometers; In all previous molecular ISM discoveries made at millimeter and centimeter wavelengths, radio telescopes of one dish were, at least partially, responsible for detection. Health and safety Effects Concentrated acetic acid corrodes the skin. These burns or blisters may appear only a few hours after exposure. Prolonged inhalation exposure (eight hours) of acetic acid vapors at 10 ppm can cause some irritation to the eyes, nose and throat; at 100 ppm there is irritation of the lungs and possible damage to the lungs, eyes and skin can result. Concentrations of 1000 ppm vapours cause noticeable irritation of the eyes, nose and upper respiratory tract and are unacceptable. These predictions were based on animal experiments and industrial impacts. Twelve workers exposed to acetic acid in the air for two years or more have an estimated 51 ppm (estimated) symptoms of conjunctival irritation, upper respiratory irritation and hyperkeratotic dermatitis. Exposure to 50 ppm or more is unbearable for most people and leads to intense lacriming and irritation of the eyes, nose and throat, with pharyngeal swelling and chronic bronchitis. Unacclimatised people experience extreme irritation of the eyes and nose at concentrations of over 25 ppm, and conjunctivitis from concentrations below 10 ppm has been reported. In the study five workers were exposed for seven to 12 years of concentrations of 80 to 200 ppm at peaks, the main findings were blackening and hyperkeratosis of the skin of the hands, conjunctivitis (but without damage to the cornea), bronchitis and pharyngitis, and erosion of open teeth (cutters and fangs). The dangers of acetic acid solutions depend on concentration. The following table lists the EU classification of acetic acid solutions: .16-14.99 mol/L Corrosive (C) R34 qgt;90% zgt;14.99 mol/L Corrosive (C) Combustible (F) R10, R35 Concentrated acetic acid can only ignite with difficulty with standard temperature and pressure, but becomes a flammable risk at temperatures over 39 degrees Celsius (102 degrees Fahrenheit), and can form explosive air mixes at higher temperatures (explosive limits: 5.4-16%). 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International Chemical Safety Map 0363 National Pollutant Inventory - NIOSH Pocket Guide to Chemical Hazards Method for Sampling and Analysis 29 CFR 1910.1000, Table No-1 (Permissible U.S. Exposure Limits) ChemSub Online: Calculating para pressure acetic acid, fluid density, dynamic fluid viscosity, surface tension of acetic acid acetic acid associated with proteins in PDB by the Swedish Chemical Agency. Information sheet – Acetic Acid Process Flow sheet of Acetic acid Production by the Carbonylation of Methanol Retrieved from 2 Gondoic acid[1] Names IUPAC name (Z)-Eicos-11-enoic acid Other names Gondoic acidcis-Gondoic acidcis-11-Eicosenoic acid11-Eicosenoic acid11Z-Eicosenoic acidcis-11-Icosenoic acid(11Z)-Icos-11-enoic acid Identifiers CAS Number 5561-99-9 Y 3D model (JSmol) Interactive imageInteractive image ChEBI CHEBI:32425 Y ChemSpider 4445895 Y KEGG C16526 Y PubChem CID 5282768 UNII UDX6WPL94T Y CompTox Dashboard (EPA) DTXSID30970949 InChI InChI=1S/C20H38O2/c1-2-3-4-5-6-7-8-9-10-11-12-13-14-15-16-17-18-19-20(21)22/h9-10H,2-8,11-19H2,1H3,(H,21,22)/b10-9- YKey: BITHHVVYSMSWAG-KTKRTIGZSA-N YInChI=1/C20H38O2/c1-2-3-4-5-6-7-8-9-10-11-12-13-14-15-16-17-18-19-20(21)22/h9-10H,2-8,11-19H2,1H3,(H,21,22)/b10-9-Key: BITHHVVYSMSWAG-KTKRTIGZBC SMILES CCCCCCCCC=CCCCCCCCCCC(=O)OO=C(O)CCCCCCCCC\C=C/CCCCCCCC Properties Chemical formula C20H38O2 Molar mass 310.51 g/mol Density 0.883 g/mL Melting point 23 to 24 °C (73 to 75 °F; 296 to 297 K) Hazards Flash point 110 °C (230 °F; 383 K) Except where otherwise noted , data is given for materials in their standard state (at 25 degrees Celsius, 100 kPa). Y check (what is yn?) Infobox references 11-Eicosenoic acid, also called gondonic acid, is a monounsaturated omega-9 fatty acid found in a variety of vegetable oils and nuts; particularly jojoba oil. It is one of several eicosenoic acids. References to cis-11-Eicocenoic acid in Sigma Aldrich and Miwe, Thomas (1971). Jojoba wax oil esters and derivative fatty acids and alcohols: gas chromatographic analyses. In the Journal of the American Society 48 (6): 259–264. doi:10.1007/bf02638458. S2CID 1466516. Received on May 6, 2013. This article on organic connectivity is a stub. You can help by expanding it.vte extracted from production of acetic acid by fermentation process. production of acetic acid by fermentation. production of acetic acid from ethanol. production of acetic acid slideshare. production of acetic acid by microorganisms. production of acetic acid from methanol. production of acetic acid pdf. production of acetic acid through microbial fermentation

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